Name: __KEY______________________ Section: ________
Chapter 4 Worksheet Spring 2007 page 1 of 4
Chapter 4 Practice Worksheet:
Reactions in Aqueous Solutions
1. List the three general classes of chemical reactions: precipitation, acid-base neutralization, and
redox reactions
2. How can you identify each of the three reaction types above (e.g., what characteristic defines
each one?)?
Precipitation reactions have solid products, also all reactants and products are ionic compounds;
Acid-base reactions react an acid with a base to produce a salt (ionic compound) and water;
Redox reactions result in a change in oxidation numbers of two species.
3. List one strong electrolyte from Table 4.1 and describe/draw how it reacts when placed in water.
Completely dissociates in water. Ex: NaCl will dissolve to produce Na
+
ions (surrounded by
water) and Cl
-
ions (surrounded by water). When salt dissolves in water, the ions separate
from each other to form a solution that conducts an electrical current.
4. List one weak electrolyte from Table 4.1 and describe/draw how it reacts when placed in water.
Only partially dissociates in water. Ex: Most molecules of HF will stay bonded together but
some will dissociate to produce H
+
ions (surrounded by water) and F
-
ions (surrounded by
water).
5. List one nonelectrolyte from Table 4.1 and describe/draw how it reacts when placed in water.
Does not dissociate in water. Ex: C
6
H
12
O
6
will stay bonded together as a complete molecule
when placed in water. When sugar dissolves in water, molecules become separated from
each other, but the molecules themselves remain intact.
6. Determine if the following compounds will be soluble or insoluble in water:
CrPO
4
insoluble (s)
Na
2
S soluble (aq)
PbBr
2
insoluble (s)
Ag
2
SO
4
insoluble (s)
Ca(ClO
3
)
2
soluble (aq)
K
3
PO
4
soluble (aq)
For the following double-displacement reactions, complete the equation and determine if there are
any insoluble products (precipitates). If there is a precipitate, write the balanced ionic and net ionic
equations. If there is no precipitate, write the balanced molecular and ionic equations.
7. NaBr (aq) + KI (aq) NaI (aq) + KBr (aq)
No net ionic equation
